Random
the shorter the bond, the ____ the bond
stronger
What is the pH of a solution that contains 2.1M strong acid?
pH= -log(2.1) = -0.32
What is the definition of a Bronsted Lowry (B.L.) acid and base?
BL acid is a proton donator
BL base is a proton receptor
Write the reaction with water for the weak base of F-
F-(aq) +H2O(l) <=> HF(aq) + OH-(aq)
Fill in the blank
pH of aqueous solution is 7 anion is derived from a ____
pH of aqueous solution is <7 canion is derived from a ____
pH of aqueous solution is >7 anion is derived from a ____
strong acid
weak base
weak acid
What is the pH of a 2.8M NH4Cl solution given the Kb for NH3 is 1.8*10^-5?
(acidic solution)
Ka= (1*10^-14)/(1.8*10^5) = 5.6*10^-10 = (x^2) / 1.5-x [basically 0]
x= square root (5.6*10^-10)(2.8) = 0.00003959797 =[H+]
pH= -log(0.00003959797) = 4.4023 = 4.40
What is the definition of a Lewis acid and base?
Lewis acid is a lone pair acceptor
Lewis base is a lone pair acceptor
Write the ionization reaction in water for hydrobromic
(Hint: strong acid)
HBr (aq) + H2O (l) =Br- (aq) + H3O+ (aq)
Label each acidic, basic, or neutral
Ka<Kb pH>7
Ka>Kb pH<7
Ka=Kb pH=7
basic
acidic
neutral
Calculate the Ka for HOI given that a a 1.7M solution has a pH of 6.42
[H+]= 10^(-6.42) = 3.80189396e-7M
Ka= (3.80189396e-7^2)/ (1.7- 3.80189396e-7) = 8.502589e-14
What must a Bronsted Lowry base have?
base must have a lone pair of electrons to accept H+
Write the ionization rxn in water for sodium hydroxide
Strong base
NaOH (aq) + H2O (l)= Na+(aq) +OH- (aq)
___ acids and ___ bases completely ionize; therefore they do not have equilibrium constants, K
strong acids, strong bases
Calculate the pH of a 1.9M NaCN solution given the Ka for HCN is 6.2*10^-10
(basic solution)
Kb= (1*10^-14)/(6.2*10^-10) = 1.6*10^10 = x^2/ 1.9- x [basically 0]
x= square root (1.6*10^-10)(1.9) = 3.04e-10 =[H+]
pH= -log(3.04e-10) = 9.5171 = 9.52
What must a Lewis acid have?
acid must have an empty orbital to accept the lone pair
Write the ionization rxn for the weak acid of hypochlorous (HClO)
HClO(aq)+H2O(l) <=> ClO-(aq)+H3O+(aq)
Something is more acidic based on:
(Hint: theres 3 fractors)
-Size
-Electronegativity
-Resonance stability
Calculate the Kb for (C2H5)3N, given a 1.2 solution that has a pH of 13.14
(basic solution)
pOH= 14-13.14 = 0.86
[OH=]= 10^-0.86 = 0.138038426M
Kb= (0.138038426^2)/(1.2-0.138038426) = 0.01794284041 = 0.018
Kw=?
Kw= Ka x Kb
Kw= 1.0*10^-14
Write the ionization for the weak base of methylamine (CH3NH2)
CH3NH2 (aq)+ H2O (l) <=> CH3H5NH3+ (aq) + OH- (aq)